This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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To balance the equation aH_2S + bSO_2 → cS + dH_2O, we need to ensure the number of atoms for each element is the same on both sides of the reaction. Step 1: Write down the number of atoms for each element on both sides of the equation using the coefficients a, b, c, d. For Hydrogen (H): Reactants: 2a Products: 2d Equation: 2a = 2d a = d For Sulfur (S): Reactants: a (from H_2S) + b (from SO_2) Products: c (from S) Equation: a + b = c For Oxygen (O): Reactants: 2b (from SO_2) Products: d (from H_2O) Equation: 2b = d Step 2: Solve the system of equations. We have: 1) a = d 2) a + b = c 3) 2b = d Substitute equation (3) into equation (1): a = 2b Now substitute a = 2b into equation (2): 2b + b = c c = 3b So, we have the relationships: a = 2b c = 3b d = 2b Step 3: Choose the smallest integer value for b to find the coefficients. Let b = 1. Then: a = 2(1) = 2 c = 3(1) = 3 d = 2(1) = 2 Step 4: Check the balanced equation with these coefficients. The balanced equation is 2H_2S + 1SO_2 → 3S + 2H_2O. Reactants: H: 2 × 2 = 4 S: 2 × 1 + 1 × 1 = 3 O: 1 × 2 = 2 Products: H: 2 × 2 = 4 S: 3 × 1 = 3 O: 2 × 1 = 2 All atoms are balanced. Step 5: Compare with the given options. The calculated coefficients are a=2, b=1, c=3, d=2. This matches option A. The final answer is A. a=2, b=1, c=3, d=2. That's 2 down. 3 left today — send the next one.